Chemistry

Question

Complete combustion of a 0.600-g sample of a compound in a bomb calorimeter releases 24.0 kJ of heat. The bomb calorimeter has a mass of 1.30 kg and a specific heat of 3.41 J/(gi°C). If the initial temperature of the calorimeter is 25.5°C, what is its final temperature?

A.30.9°C
B.34.5°C
C.44.0°C
D.51.5°C

2 Answer

  • Data:

    Heat = 24 KJ = 24,000 J
    mass = 1.3kg = 1300 g
    Cs = 3.41 J / (g °C)
    Ti = 25.5 °C
    Question: Tf


    Formula: Heat = mCsΔT =>

    ΔT = Heat / (mCs) = 24000J/[1300g*3.41J/(g°C)] = 5.4 °C

    ΔT = Tf - Ti => Tf = ΔT + Ti = 25.5°C + 5.4°C = 30.9°C

    Answer: 30.9°C
  • The final temperature of the calorimeter is 30.9 °C (Option A)

    Data obtained from the question

    • Heat (Q) = 24 KJ = 24 × 1000 = 24000 J
    • Mass (M) = 1.30 kg = 1.3 × 1000 = 1300 g
    • Specific heat capacity (C) =  3.41 J/gºC
    • Initial temperature (T₁) = 25.5 °C
    • Final temperature (T₂) =?

    How to determine the final temperature

    The final temperature of the calorimeter can be obtained as illustrated below:

    Q = MC(T₂ – T₁)

    24000 = 1300 × 3.41 (T₂ – 25.5)

    24000 = 4433 (T₂ – 25.5)

    Divide both side by 4433

    24000 / 4433 = T₂ – 25.5

    5.4 = T₂ – 25.5

    Collect like terms

    T₂ = 5.4 + 25.5

    T₂ = 30.9 °C

    Thus, the final temperature of the calorimeter is 30.9 °C

    Learn more about heat transfer:

    https://brainly.com/question/6363778

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